Ammonia and Nitric Acid (school Names) — Hno3 and Nitrates

HNO₃ → nitrate salts. Examples: NaNO₃, KNO₃, NH₄NO₃. The nitrate ion is NO₃⁻; the nitrite ion is NO₂⁻ — they are different.

Nitric acid is manufactured industrially from ammonia through the Ostwald Process. It behaves as a strong acid in aqueous solution. Reaction with a suitable base produces a nitrate salt and water. For example: HNO₃ + NaOH → NaNO₃ + H₂O. Nitrates are important in agriculture and chemical manufacture. Ammonium nitrate NH₄NO₃ is an important nitrogen fertilizer. Nitric acid is also an oxidizing acid, especially when concentrated, so its reactions with metals can differ from the simple behaviour expected for non-oxidizing dilute acids. Do not confuse nitrate NO₃⁻ with nitrite NO₂⁻.

Nitric acid is HNO₃. Its salts are nitrates, containing NO₃⁻. Ostwald Process makes nitric acid from ammonia. Ammonium nitrate is a fertilizer.

Nitrates contain NO₃⁻. Neutralization with NaOH gives sodium nitrate. Ostwald starts from ammonia, not from Haber as the final nitric-acid product.

Nitric acid's oxidizing behaviour means metal reactions should not automatically be predicted using the simple acid + metal → hydrogen rule. Nitrite NO₂⁻ is a different ion.

NO₃⁻ = nitrate ion. Ostwald → HNO₃. Nitrite ≠ nitrate.